Input interpretation
![hydrazoic acid](../image_source/25f155dfdec40f882d53a98b405306ef.png)
hydrazoic acid
Chemical names and formulas
![formula | HNN congruent N Hill formula | HN_3 name | hydrazoic acid IUPAC name | diazonioazanide alternate names | diazoimide | hydrogen azide | triazoic acid mass fractions | H (hydrogen) 2.34% | N (nitrogen) 97.7%](../image_source/2b0b04e639447b05c2133db34ff7d703.png)
formula | HNN congruent N Hill formula | HN_3 name | hydrazoic acid IUPAC name | diazonioazanide alternate names | diazoimide | hydrogen azide | triazoic acid mass fractions | H (hydrogen) 2.34% | N (nitrogen) 97.7%
Lewis structure
![Draw the Lewis structure of hydrazoic acid. Start by drawing the overall structure of the molecule, ignoring potential double and triple bonds: Count the total valence electrons of the hydrogen (n_H, val = 1) and nitrogen (n_N, val = 5) atoms: n_H, val + 3 n_N, val = 16 Calculate the number of electrons needed to completely fill the valence shells for hydrogen (n_H, full = 2) and nitrogen (n_N, full = 8): n_H, full + 3 n_N, full = 26 Subtracting these two numbers shows that 26 - 16 = 10 bonding electrons are needed. Each bond has two electrons, so in addition to the 3 bonds already present in the diagram add 2 bonds. To minimize formal charge nitrogen wants 3 bonds. Identify the atoms that want additional bonds and the number of electrons remaining on each atom: To fully fill its valence shell, nitrogen will donate one of its electrons, allowing it to form four bonds (the maximum number an element on period 2 can form). Fill in the 2 bonds by pairing electrons between adjacent highlighted atoms, noting the formal charges of the atoms: Answer: | |](../image_source/3c91b38a9b3e48c29ed746a1162cb3a1.png)
Draw the Lewis structure of hydrazoic acid. Start by drawing the overall structure of the molecule, ignoring potential double and triple bonds: Count the total valence electrons of the hydrogen (n_H, val = 1) and nitrogen (n_N, val = 5) atoms: n_H, val + 3 n_N, val = 16 Calculate the number of electrons needed to completely fill the valence shells for hydrogen (n_H, full = 2) and nitrogen (n_N, full = 8): n_H, full + 3 n_N, full = 26 Subtracting these two numbers shows that 26 - 16 = 10 bonding electrons are needed. Each bond has two electrons, so in addition to the 3 bonds already present in the diagram add 2 bonds. To minimize formal charge nitrogen wants 3 bonds. Identify the atoms that want additional bonds and the number of electrons remaining on each atom: To fully fill its valence shell, nitrogen will donate one of its electrons, allowing it to form four bonds (the maximum number an element on period 2 can form). Fill in the 2 bonds by pairing electrons between adjacent highlighted atoms, noting the formal charges of the atoms: Answer: | |
3D structure
![3D structure](../image_source/70441faba33e8c5eb7bc42f648a92862.png)
3D structure
Basic properties
![molar mass | 43.029 g/mol](../image_source/80b6ae45c05b93408157d5d3b5c1af2b.png)
molar mass | 43.029 g/mol
Units
Chemical identifiers
![CAS number | 7782-79-8 PubChem CID number | 24530 SMILES identifier | N=[N+]=[N-] InChI identifier | InChI=1S/HN3/c1-3-2/h1H](../image_source/e57248452cfbbe7e62471f66d33481c5.png)
CAS number | 7782-79-8 PubChem CID number | 24530 SMILES identifier | N=[N+]=[N-] InChI identifier | InChI=1S/HN3/c1-3-2/h1H
Toxicity properties
![threshold limit value | 0.11 ppmv](../image_source/8de4da7ea56e345b17efba62218ffdb9.png)
threshold limit value | 0.11 ppmv
Units